Answer:1. Enter the following quantities from Part of the experiment, making sure to use the correct units and correct number of significant figures. a. Mass of beaker b. Volume M NaCl added c. Number of moles of NaCl added to the beaker (theoretical yield): d. Mass beaker + salt e. Number of moles of NaCl recovered (actual yield): f. What is your percent yield for NaCl? 2. In Experiment A, what could cause you to have a percent yield less than 100%?
3. In experiment A, what could cause you to have a percent yield greater than 100%? 4. Enter the following quantities from Part B: Trial 1, making sure to use the correct units and correct number of significant figures a. Mass of the beaker b. Mass of the sodium bicarbonate added to the beaker: Mace at the healer alt for aurat
Call Out OWL c. Mass of the beaker + salt after evaporation: d. Mass of the salt remaining in the beaker after evaporation: 5. Enter the following quantities from Part B: Trial that you calculated on your calculation sheet, making sure to use the correct units and correct number of significant figures. a. How many moles sodium bicarbonate (baking soda) were added to the beaker? b. How many moles NaCl would be made from the moles of sodium bicarbonate added to the beaker? c. How many grams of NaCI would theoretically be made in the reaction of sodium bicarbonate and HCI? d. What is the percent yield in Trial I?
6. Enter the following quantities from Part B: Trial 2, making sure to use the correct units and correct number of significant figures. a. Mass of the beaker b. Mass of the sodium bicarbonate added to the beaker: c. Mass of the beaker + salt after evaporation: d. Mass of the salt remaining in the beaker after evaporation: 7. Enter the following quantities from Part B: Trial 2 that you calculated on your calculation sheet, making sure to use the correct units and correct number of significant figures a. How many moles sodium bicarbonate (baking soda) were added to the beaker? b. How many moles NaCl would be made from the moles of sodium bicarbonate added to the beaker? c. How many grams of NaCl would theoretically be made in the reaction of sodium bicarbonate and HCI?
3/4 5 d. What is the percent yield in Trial 2? 8. How do you determine the reaction of the baking powder and HCl is complete? 9. Choose one of your trial results for the Stoichiometry of a Reaction that is not 100% Give a reasonable explanation why you saw that result 12:15 PM
The molecular formula is C₄H₈O.
We must <em>calculate the masses</em> of C, H, and O from the masses given.
Mass of C = 17.873 mg CO₂ × (12.01 mg C/44.01 mg CO₂) = 4.8774 mg C
Mass of H = 7.316 mg H₂O × (2.016 mg H/18.02 mg H₂O) = 0.818 48 mg H
Mass of O = Mass of compound - Mass of C - Mass of H
= (7.321 – 4.8774 – 0.818 48) mg = 1.6251 mg
Now, we must convert these <em>masses to moles</em> and <em>find their ratios</em>.
From here on, I like to summarize the calculations in a table.
<u>Element</u> <u> </u><em><u>m</u></em><u>/mg </u> <em><u>n</u></em><u>/mmol</u> <u> Ratio </u> <u>Integers</u>
C 4.877 4 0.406 11 3.9984 4
H 0.818 48 0.811 99 7.9944 8
O 1.625 1 0.101 57 1 1
The empirical formula is C₄H₈O.
Answer:
The formal charge for H,O,F,O = 0 ,0 , 1, -1
Explanation:
The octet of electrons acquired by oxygen and fluorine atoms in this structure and the formal charges add to zero.Assigning of a formal charge +1 to an electro-negative atom as fluorine indicates that a structure does not occur .Fluorine normally forms one oxyacid HOF.
The equation of state for a hypothetical ideal gas is known as the ideal gas law, sometimes known as the general gas equation. i.e. PV = nRT or P1V1 = P2V2.
- According to the ideal gas law, the sum of the absolute temperature of the gas and the universal gas constant is equal to the product of the pressure and volume of one gram of an ideal gas.
- Robert Boyle, Gay-Lussac, and Amedeo Avogadro's observational work served as the basis for the ideal gas law. The Ideal gas equation, which simultaneously describes every relationship, is obtained by combining all of their observations into a single statement.
- When applying the gas constant R = 0.082 L.atm/K.mol, pressure, volume, and temperature should all be expressed in units of atmospheres (atm), litres (L), and kelvin (K).
- At high pressure and low temperature, the ideal gas law basically fails because molecule size and intermolecular forces are no longer negligible but rather become significant considerations.
Learn more about ideal gas law here:
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The Iron (III) ion is
The sulfate ion is
Thus when forming the compound iron (iii) sulfate you would need three sulfate ions bonded to two iron ions in order to fill the valency requirement
∴ the formula would be Fe₂(SO₄)₃
Whenever you are adding a number to a radical you must bracket it.